What is the Difference Between Transition Metals and Inner Transition Metals?

Transition metals and inner transition metals are two groups of elements in the periodic table that have some similarities but also significant differences in their atomic structure and chemical properties. The main differences between them are:

1. Atomic Structure: Both transition and inner transition metals have the same atomic structure, but the electrons fill their orbitals in different ways. Transition metal atoms have their valence electrons in the outermost d orbital, while inner transition metal atoms have them in the inner penultimate f orbital.
2. Location in the Periodic Table: Transition metals are found in groups 3-12 of the periodic table, while inner transition metals are in the f-block, specifically in the lanthanides and actinides groups.
3. Electronegativity: Transition elements generally relinquish two electrons, while inner transition elements, particularly the lanthanides, tend to surrender all three electrons in their outermost shells.
4. Size of the Atom: Inner transition metals also give up their electrons more easily than transition metals, which affects the size of the atom.
5. Chemical Properties: The two groups of inner transition elements, actinides and lanthanides, behave differently from each other, even though they are both considered rare earth elements. Lanthanides are soft, malleable, ductile, and chemically reactive elements that burn easily in air and have many industrial uses. Actinides are a series of chemically similar metallic elements that are all radioactive, with some, like uranium and plutonium, being used to generate nuclear energy.

Comparative Table: Transition Metals vs Inner Transition Metals

Transition metals and inner transition metals are two groups of elements in the periodic table that have some similarities but also significant differences. Here is a table comparing their main characteristics:

Transition metals are located in the d block of the periodic table and have valence electrons in their s, p, d, and f orbitals. They are characterized by their ability to easily lose electrons and form stable cations. Examples of transition metals include iron, copper, and zinc.

Inner transition metals, on the other hand, are located in the f block of the periodic table and have valence electrons in their f orbitals. They consist of two series: lanthanides (atomic numbers 57-71) and actinides (atomic numbers 89-103). Inner transition metals are larger in size due to their high number of electron shells and have more unpaired electrons, even in their stable cations. They also tend to give up their electrons more easily than transition metals, commonly relinquishing three electrons instead of two.